# Question 88d69

May 8, 2017

The sample contains 0.11 mol of ${\text{CO}}_{2}$.

#### Explanation:

We can use the Ideal Gas Law to solve this problem:.

$\textcolor{b l u e}{\overline{\underline{| \textcolor{w h i t e}{\frac{a}{a}} p V = n R T \textcolor{w h i t e}{\frac{a}{a}} |}}} \text{ }$

We can rearrange this equation to get

$n = \frac{p V}{R T}$

STP is defined as 1 bar and 0 °C.

Thus,

$p = \text{1 bar}$
$V = \text{2.5 L}$
$R = \text{0.083 14 bar·L·K"^"-1""mol"^"-1}$
$T = \text{(0 + 273.15) K" = "273.15 K}$

n = (1 color(red)(cancel(color(black)("bar"))) × 2.5 color(red)(cancel(color(black)("L"))))/("0.083 14" color(red)(cancel(color(black)("bar·L·K"^"-1")))"mol"^"-1" × 273.15 color(red)(cancel(color(black)("K")))) = "0.11 mol"#